Hydrogen peroxide can be prepared by the reaction of barium peroxide with sulfuric acid according to the reaction bao2(s)+h2so4(aq)⟶baso4(s)+h2o2(aq) how many milliliters of 4.00 m h2so4(aq) are needed to react completely with 32.7 g bao2(s)?

The answer to your question is: Volume = 15.2 ml

Explanation:

Data

H2SO4 4M  = ?

BaO2          = 32.7 g

                        BaO2(s)  +  H2SO4(aq)  ⟶  BaSO4(s)  +  H2O2(aq)

MW BaO2 = 137 + 32 = 169 g

MW H2SO4 = 2 + 32 + 64 = 98 g

                       169 g of BaO2  98 g of H2SO4

                        32.7 g of BaO2    x

                        x = (32.7 x 98)/ 169

                        x = 18.99 ≈ 19 g of H2SO4

Density of H2SO4 = 1.25 g/lml

Volume = mass / density

Volume = 19 g / 1.25 g/ml

Volume = 15.2 ml

answer: -

reaction:

na + cl ⇌ nacl

balanced chemical equation:

na + 2cl ⇌ nacl2

sodium + clorine goes to form sodium chloride (table salt).

the product is nacl2.

and the reactants are na and cl.

(note: if you don’t know what ⇌ means, read below: -

⇌(double head arrow) means reversible reaction).